Discussion
If \(f\) represents the intermolecular force between molecules and \(V\), is the volume occupied by the gas molecules, then at high pressure and at low temperatures, the gas shows large deviation from the ideal behaviour because the fact that
Answer: E
The reason is that f is appreciable and V is not negligible.
The ideal gas model assumes there are no intermolecular forces and that the molecules' own volume is negligible. At high pressure and low temperature the molecules are crowded together and move slowly, so attractive forces become significant and the molecules' own volume is a sizeable part of the total.
Both assumptions fail, which is why van der Waals added the corrections a and b. The options saying f or V is negligible describe the conditions in which a gas behaves ideally.
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